Use Stirling's approximation to show that the multiplicity of an Einstein solid, for any large values ofNandlocalid="1650383388983" q,is approximately

Omega(N,q)q+Nqqq+NNN2πq(q+N)/N

The square root in the denominator is merely large, and can often be neglected. However, it is needed in Problem2.22. (Hint: First show thatΩ=Nq+N(q+N)!q!N!. Do not neglect the2πNin Stirling's approximation.)

Short Answer

Expert verified

The square root and the large values are neglect

Ω(N,q)q+Nqqq+NNN2πq(q+N)N

Step by step solution

01

Macroscopic solid

For any macroscopic solid, both qand Nare large numbers (on the order of Avogadro's number, or1023) so the factorials in Ωare very large numbers, not calculable on most computers. To get estimates of Ωwe can use Stirling's approximation for the factorials. The multiplicity is given by:

Ω(N,q)=q+N-1q

Writing out the binomial coefficient:

q+N-1q=(q+N-1)!q!(N-1)!

we can write the factorial (q+N-1)! in the following form:

(q+N-1)!=(q+N-1)!×q+Nq+N

we can write the factorial (q+N-1)! in the following form:

(q+N-1)!=(q+N-1)!×q+Nq+N

but,(q+N-1)!(q+N)=(q+N)so

(q+N-1)!=(q+N)!(q+N)

and also we can write the factorial (N-1)! in the following form:

(N-1)!=(N-1)!×NN=N!N

Assume that qand Nare large numbers, so:

02

Substitution 

substitute from (2) and (3) into (1), so:

Ω(N,q)=q+N-1q=N(q+N)(q+N)!N!q!

Assume that qand Nare large numbers, so we can use Stirling's approximation for the factorials:

n!2πnnne-n

so we get:

N!2πNNNe-Nq!2πqqqe-q(q+N)!2π(q+N)(q+N)(q+N)e-(q+N)

substitute from (5),(6)and (7)into (4), so:

Ω(N,q)N(q+N)2π(q+N)(q+N)(q+N)e-(q+N)2πNNNe-N2πqqqe-q

cancel e^{-(q+N)}withe^{-q}e^{-N}so:

Ω(N,q)N(q+N)2π(q+N)(q+N)(q+N)2πNNN2πqqq

Ω(N,q)N2π(q+N)(q+N)(2πq)(2πN)(q+N)(q+N)NNqq

Ω(N,q)N2πq(q+N)(q+N)(q+N)NNqq

03

Substitution 

but, (q+N)^{(q+N)}=(q+N)^{q}(q+N)^{N}, so:

Ω(N,q)N2πq(q+N)(q+N)q(q+N)NNNqq

Ω(N,q)N2πq(q+N)q+Nqqq+NNN

Ω(N,q)q+Nqqq+NNN2πq(q+N)N

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Describe a few of your favorite, and least favorite, irreversible processes. In each case, explain how you can tell that the entropy of the universe increases.

According to the Sackur-Tetrode equation, the entropy of a monatomic ideal gas can become negative when its temperature (and hence its energy) is sufficiently low. Of course this is absurd, so the Sackur-Tetrode equation must be invalid at very low temperatures. Suppose you start with a sample of helium at room temperature and atmospheric pressure, then lower the temperature holding the density fixed. Pretend that the helium remains a gas and does not liquefy. Below what temperature would the Sackur-Tetrode equation predict that Sis negative? (The behavior of gases at very low temperatures is the main subject of Chapter 7.)

For a single large two-state paramagnet, the multiplicity function is very sharply peaked about N=N/2.

(a) Use Stirling's approximation to estimate the height of the peak in the multiplicity function.

(b) Use the methods of this section to derive a formula for the multiplicity function in the vicinity of the peak, in terms of xN(N/2). Check that your formula agrees with your answer to part (a) when x=0.

(c) How wide is the peak in the multiplicity function?

(d) Suppose you flip 1,000,000coins. Would you be surprised to obtain heads and 499,000 tails? Would you be surprised to obtain 510,000 heads and 490,000 tails? Explain.

Rather than insisting that all the molecules be in the left half of a container, suppose we only require that they be in the leftmost 99%(leaving the remaining 1%completely empty). What is the probability of finding such an arrangement if there are 100molecules in the container? What if there are 10,000molecules? What if there are 1023?

For either a monatomic ideal gas or a high-temperature Einstein solid, the entropy is given by times some logarithm. The logarithm is never large, so if all you want is an order-of-magnitude estimate, you can neglect it and just say . That is, the entropy in fundamental units is of the order of the number of particles in the system. This conclusion turns out to be true for most systems (with some important exceptions at low temperatures where the particles are behaving in an orderly way). So just for fun, make a very rough estimate of the entropy of each of the following: this book (a kilogram of carbon compounds); a moose of water ; the sun of ionized hydrogen .

See all solutions

Recommended explanations on Physics Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free